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CHALLENGE: describe and explain the shape of the successive IE graph for Aluminium

small increase from 1 to 2 and 2 to 3 as in each case, less e- than p+ so e- more attracted; BIG jump from 3 to 4 as the fourth e- to be removed is in the shell 2 (the inner shell) so far more attracted

When a transition metal forms an ion, why are the 4s sub shell electrons lost before the 3d sub shell?

SCARED: Nuclear charge, distance from the nucleus (nuclear attraction), shielding, whether the orbital contains a pair of electrons leading to electron repulsion or a singularly occupied orbital.

CHALLENGE: Which is highest of 1st IE of Na or 2ndIE of Mg?

No brainer! Magnesium: 1st IE of Mg is bigger than 1st IE of Na because there are more protons in Mg (same shielding, same distance, same shell etc...). And the 2nd IE of any element is always higher than the 1st one.

CHALLENGE: Which is highest of 3rd IE of Al or 3rd IE of Mg?

Magnesium: In the successive IE graph, an element STARTS the big jump on the group number. So Mg will have a big increase in IE between 2 and 3rd IE: the 3IE will be very high. Aluminium will not have had the big jump yet...

What is the electronic configuration of Copper +2 ions

always start with the electron configuration of the ATOM: [Ar] 3d9 4s2 (did you remember that copper is an exception?); then remove the 4s: [Ar] 3d9

What is the electronic configuration of Iron+2 ions

always start with the electron configuration of the ATOM: [Ar] 3d6 4s2; then remove the 4s first: [Ar] 3d6